1. ATOMIC STRUCTURE QUARTER 1, UNIT 1

2. HOW SMALL IS AN ATOM? http://htwins.net/scale2/?bordercolor=white

3. THE ATOM BASKETBALL Atoms are mostly Protons Neutrons Electrons orbital What force keeps electrons orbiting? Electromagnetic force What force keeps protons in the nucleus? Nuclear fussion

4. THE “ATOM” BOMB ON HIROSHIMA President Truman End of WW2, Beginning of Cold War

5. Identify the location, relative mass, and charge for electrons, protons, and neutrons. Describe the atom as mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus. Recognize that protons repel each other and that a strong force needs to be present to keep the nucleus intact.

6. THE FACEBOOK PROFILE OF AN ELEMENT Elements are identified by the number of protons they have. Amount of neutrons change: Isotope Atomic Mass: http://www.wikihow.com/Calculate-Atomic-Mass http://www.wikihow.com/Calculate-Atomic-Mass Amount of electrons change: Ion

7. CALCULATING ATOMIC MASS http://www.ptable.com/

8. YSBAT: List the number of protons, neutrons, and electrons for any given ion or isotope. Recognize that an element always contains the same number of protons.

9. PROPERTIES FORM OF ELEMENTS

10. HAPPINESS IS A JOURNEY NOT A DESTINATION

11. PERIODIC TRENDS QUARTER 1 UNIT 1

12. http://www.ptable.com/#Orbital

13. ALL PERIODIC TRENDS CAN BE UNDERSTOOD IN TERMS OF THREE BASIC RULES. 1.Electrons are attracted to the protons in the nucleus of an atom. 2.Shielding: 3.Completed shells are stable.

14. WE TEND TO FORGET PERIODIC TRENDS …

17. YSBAT… Identify elements with similar chemical and physical properties using the periodic table.

18. QUESTION ONE The most electronegative element?  C  N  O  F  Ne Think about the trend for electronegativity: Farthest right and farthest up. Fluorine who only needs one electron to fill its shell. The smallest radius of that group also. Do not count the noble gases because they are already satisfied.

19. QUESTION TWO Which of the following ions has the smallest ionic radius?  O 2-  F-  Na +  Mg 2+  Al 3+ As an element loses its electrons the radius decreases. Electrons are held more tightly. Al 3+ has the most protons, so the electrons experience greater attractive force from the nucleus.

20. QUESTION THREE Which of the following statements is true regarding sodium and chlorine?  Sodium has greater electronegativity and a larger first ionization energy.  Sodium has a larger first ionization energy and a larger atomic radius.  Chlorine has a larger atomic radius and a greater electronegativity.  Chlorine has a greater electronegativity and a larger first ionization energy.  Chlorine has a larger atomic radius and a larger ionization energy.

21. QUESTION 4 Which of the following nuclei has 3 more neutrons than protons?  B with the atomic mass of 11  Cl with the atomic mass of 37  Mg with the atomic mass of 24  Ga with the atomic mass of 70  F with the atomic mass of 19  37 -17 Protons = 20 Neutrons.  20 Neutrons- 17 protons= 3 neutrons.

22. QUESTION 5 Give the number of electrons and protons if the fluoride ion has a -1 charge. # of protons_____ # of electrons______ Fluorine has 9 protons – 10 electrons= -1

23. QUESTION 6 Identify parts of a atom

24. QUESTION 7 Like a basketball, the atom is described as mostly empty space with an extremely small, dense nucleus consisting of the protons and electrons and an electron cloud surrounding the nucleus.

25. QUESTION 8 Knowing that protons repel each other, name and describe the strong force that keeps the nucleus intact? Nuclear fusion is when the protons and neutrons share each others mass. This creates a strong attraction with a lot of energy.

26. QUESTION 9 The ionization energies for an element are listed in the table below. FirstSecondThirdFourthFifth 8 eV15 eV80 eV109 eV 141 eV Based on the ionization energy table, the element is most likely to be Sodium (Na). Magnesium (Mg). Aluminum (Al). Silicon (Si). Phosphorus (P).

27. QUESTION 10 10. Use your knowledge of the periodic table of the elements to answer the following questions. (Use the back of this paper if you need more space) Explain the trend in electronegativity for P to S to Cl. As you move across a period on the the periodic table the elements become more electronegative because the atomic radius is decreasing. Electrons are held tighter as elements approach the state of being stable. Explain the trend in atomic radius from Li to Na to K. As you move down a group on the periodic table the atomic radius increases because the number of electron orbitals are increasing and the amount of shielding that occurs within those shells is also increasing.